Chemistry 1120 Exam 3 Study Guide
Chemistry 1120 Exam 3 Study Guide Chem 1120-001
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This 8 page Study Guide was uploaded by Callie Simpson on Monday February 29, 2016. The Study Guide belongs to Chem 1120-001 at East Carolina University taught by James E. Collins in Winter 2016. Since its upload, it has received 60 views. For similar materials see Introduction to Chemistry for the Allied Health Sciences in Science at East Carolina University.
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Date Created: 02/29/16
Name: Exam 3 Study Guide Chemistry 1120 Some Useful Quantities: N = 6.02 x 10 (Avogadro's Number) R = 0.0821 L•atm/mol•K 1. Which of the following molecules in the pure liquid state would be expected to hydrogen bond? H H H O ** ** H C C H H N N H H C C H H H H H H (1) (2) (3) a) 1 only b) 2 only c) 3 only d) 2 and 3 e) All of the above 2. On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point. CHCl 3(Chloroform), CH 3H 2H C2 CH2 (P3ntane), and H O2(Water) a) (lowest bp) Penane < Chloroform < Water (highest bp) b) (lowest bp) Penane < Water < Chloroform (highest bp) c) (lowest bp) Water < Chloroform < Penane (highest bp) d) (lowest bp) Water < Penane < Chloroform (highest bp) e) (lowest bp) Chloroform < Water < Penane (highest bp) 3. The following compounds have very limited solubility in water. 1) PbB2 (solid) 2) CH2Cl2 (liquid) 3) O2 (gas) Which of the following would increase in solubility at lower temperatures and higher pressures? (Pay careful attention to their physical states.) a) 1 only b) 2 only c) 3 only d) 1 and 2 e) All of the above 4. Which of the following molecular compounds would be highly soluble in water, H2O? (Remember: "Like dissolves Like".) 1) HF 2) NH3 3) CH4 a) 1 only b) 2 only c) 3 only d) 1 and 2 e) 1 and 3 5. How many Potassium atoms are present in 10.0 grams of Potassium? a) 6.50 x 10 atoms of Potassium b) 5.14 x 10 atoms of Potassium 23 c) 1.54 x 10 atoms of Potassium d) 1.94 x 10 atoms of Potassium 26 e) 2.35 x 10 atoms of Potassium 6. What is the molar mass for Calcium nitrate? a) 54.09 g/mol b) 86.09 g/mol c) 102.09 g/mol d) 132.10 g/mol e) 164.10 g/mol 7. How many grams of sulfur are present in 100.0 grams of Al S ? 2 3 MM(Al S )2 3 150.14 g/mol a) 0.400 g of Sulfur b) 21.4 g of Sulfur c) 60.0 g of Sulfur d) 64.1 g of Sulfur e) 90.1 g of Sulfur Consider the following balanced chemical reaction to answer the next two questions: N2H 4 + 2 H 2 2 N 2 + 4H 2 32.06 g/mol 34.02 g/mol 28.02 g/mol 18.02 g/mol 8. How many moles of nitrogen, N are pr2duced when 5.00 moles of hydrogen peroxide, H O2 r2act completely? a) 2.5 moles of N b) 4.12 moles of N c) 5.00 moles of N 2 2 2 d) 6.07 moles of N 2 e) 10.0 moles of N 2 9. How many grams of N H wou2d 4e required to produce 20.0 g of H O? 2 a) 8.90 g N 2 4 b) 11.2 g N H2 4 c) 17.8 g N H2 4 d) 35.6 g N 2 4 e) 44.8 g N H2 4 10. A certain automobile tire is inflated to 36.0 pounds per square inch. What pressure is this tire reported in mm of Hg? (1 atm = 14.7 psi and 1 atm = 760 mm Hg) a) 0.696 mm of Hg b) 1.44 mm of Hg c) 2.45 mm of Hg 3 5 d) 1.86 x 10 mm of Hg e) 4.02 x 10 of Hg 11. The subscripts on the Macroscopic scale in a chemical formula for a compound represent what? a) The gram to gram ratio of the elements in the formula b) The amu to amu ratio of the atoms in the formula c) The mole to mole ratio of the elements in a formula d) The charges of each ion in the formula e) The molar mass of each element in the formula 12. A sample of COgas has a volume of 7.31 L at a pressure of 735 mm of Hg and a temperature of 45 C. What would be the temperature in degrees Celsius of this same amount of gas at a pressure of 1275 mm of Hg and a volume of 0.800 L? a) 213 C b) 8.5 C c) 60.4 C d) 333 C e) 1402 C 13. A gas is initially contained in a moveable cylinder that occupies a volume of 900. mL under a pressure of 3.00 atm. What would be the volume of this same gas if the pressure is reduced to 0.500 atm at constant temperature? 4 a) 1.86 x 10 mL b) 150 mL c) 600 mL d) 1.35 x 10 mL e) 5.40 x 10 mL 14. What is the pressure in atmospheres of 0.100 moles of O gas2in a 2.0 Liter container at a temperature of 75 C? a) 0.308 atm b) 0.700 atm c) 1.43 atm d) 3.25 atm e) 5.71 atm 15. The total pressure exerted by a mixture of the three gases, oxygen, nitrogen and water vapor is 742 mm of Hg. The partial pressure of oxygen and nitrogen in the sample are 581 mm of Hg and 143 mm of Hg respectively. What is the partial pressure of water vapor in this mixture? a) 18 mm of Hg b) 304 mm of Hg c) 724 mm of Hg d) 1180 mm of Hg e) 1466 mm of Hg 16. How would the Ideal gas Law equation be rearranged to solve for the moles of gas? Answer: b P x V R x T n = P x V x R x T n = n = R x T P x V (a) (b) (c) 1 P x V x R n = P x V x R x T n = T (d) (e) 17. Which of the following three states of matter have a definite volume but an indefinite shape? 1) Solids 2) Liquids 3) Gases a) 1 only b) 2 only c) 3 only d) 1 and 2 e) All of the above 18. What is the osmolarity of an aqueous 0.25 M Na PO 3olu4ion? a) 0.25 osmolar b) 0.50 osmolar c) 1.0 osmolar d) 1.5 osmolar e) 2.0 osmolar 19. Which of the following three states of matter have (has) forces of repulsion that are comparable to their forces of attraction? 1) Solids 2) Liquids 3) Gases a) 1 only b) 2 only c) 3only d) 1 and 2 e) All of the above 20. Which phase change listed below represents the transition from the solid state to the gaseous state? a) Condensation b) Deposition c) Evaporation d) Freezing e) Sublimation 21. Which of the following phase changes listed below would be considered exothermic? 1) Melting 2) evaporation 3) Freezing a) 1 only b) 2 only c) 3 only d) 1 and 3 e) All of the above 22. An aqueous solution of Ag SO contains 0.28 g of Ag SO dissolved in 25.0 o 2 4 2 4 grams of water at 50 C. How would this solution be described qualitatively if the solubility limit for this compound at 50 C is 1.08 g Ag SO /120 g 4f water? a) Unsaturated solution b) Saturated solution c) Supersaturated solution d) Dilute solution e) Heterogeneous solution 23. How many grams of Na CO ar2 req3ired to prepare 25.0 mL of a 2.00 %(m/v) Na 2O s3lution? a) 0.0800 g Na C2 3 b) 0.500 g Na C2 3 c) 2.00 g Na C2 3 d) 12.5 g Na 2O 3 e) 50.0 g Na 2O 3 24. How many grams of AgNO are pre3ent in 50.0 mL of a 12.0 M AgNO solution? 3 MM(AgNO ) = 3169.88 g/mol. a) 708 g of AgNO 3 b) 40.8 g of AgNO 3 c) 283 g of AgNO 3 d) 102 g of AgNO 3 e) 3.53 g of AgNO 3 25. Concentrated sulfuric acid, H SO i2 1840 M. How many milliliter of concentrated sulfuric acid, H SO 2s re4uired to prepare 500 mL of 3.00 M H SO 2 4 acid solution? 5 a) 3.70 x 10 mL b) 9.26 mL c) 83.3 mL d) 3.00 x 10 mL e) 2.70 x 10 mL 26. Arrange the following three aqueous solutions in order of decreasing freezing point. 0.50 M C H 6 12 6 0.20 M KNO 3 0.25 M MgCl 2 a) (highest fp) 0.20 M KNO > 0350 M C H O > 6.212M 6gCl (lowest fp) 2 b) (highest fp) 0.50 M C H O > 0.20 M KNO > 0.25 M MgCl (lowest fp) 6 12 6 3 2 c) (highest fp) 0.50 M C H O6 12 0625 M MgCl > 0.20 M 2NO (lowest fp) 3 d) (highest fp) 0.25 M MgCl > 0.20 M KNO > 0.50 M C H O (lowest fp) 2 3 6 12 6 e) (highest fp) 0.25 M MgCl > 0250 M C H O > 60.12 M6KNO (lowest fp) 3 27. Below is a figure of a normal red blood cell. The osmolarity of a red blood cell is approximately 0.3 osmolar. Assuming osmosis is operative, what would happen if this red blood cell is immersed in an aqueous glucose solution with a concentration less than 0.3 osmolar? a) There is a net movement of water molecules from the red blood cell into the glucose solution and the red blood cells shrinks. b) There is a net movement of water molecules from the glucose solution into the red blood cells and the red blood cells swells. c) There is a net movement of glucose molecules from the glucose solution into the red blood cell and the red blood cell swells. d) There is a net movement of solute molecules out of the red blood cell into the glucose solution and the red blood cell shrinks. e) Water exits the red blood cells and glucose enters the red blood cells resulting in no net change in total volume of the red blood cell. 28. Which of the following aqueous solutions would be considered hypotonic with respect to a red blood cell? (The Osmolarity of a red blood cell is approximately equal to 0.30 osmolar.) 1) 0.30 M glucose (molecular) 2) 0.20 M NaCl 3) Pure distilled water a) 3 only b) 1 and 3 c) 2 and 3 d) All of the above e) None of the above 29. Which of the following solutions would cause crenation of the red blood cell? 1) 0.30 M glucose (molecular) 2) 0.20 M NaCl 3) Pure distilled water a) 2 only b) 1 and 3 c) 2 and 3 d) All of the above e) None of the above 30. The solubility of oxygen in blood is 0.44 g/100 mL at a partial pressure of 159 mm Hg. What is the solubility of oxygen in blood where the partial pressure of O 2is 56 mm Hg? a) 0.15 g / 100 mL b) 0.35 g / 100 mL c) 0.80 g / 100 mL d) 1.3 g / 100 mL e) 6.5 g / 100 mL 31. What is the definition for percentage by mass (m/m)? a) (grams of solute / grams of solvent) x 100% b) (grams of solvent / grams of solute) x 100% c) (moles of solute / moles of solvent) x 100% d) (grams of solute / grams of solution) x 100% e) (moles of solution / moles of solute) x 100% Consider allowing 0.75 moles of Aluminum and 0.50 moles of chlorine to react to produce AlCl a3 shown below to answer the next two questions: 2 Al (s) + 3 Cl2 (g) 2 AlCl 3s) 32. Which substance is the limiting reactant when 0.75 moles of aluminum metal, (Al) and 0.50 moles of chlorine gas, (Cl ) 2re allowed to react as shown in the reaction below? a) Al b) Cl2 c) AlCl 3 d) None of these; they are mixed in exact proportions. 33. What is the percentage yield in a certain experiment, if 0.25 moles of AlCl were3 recovered at the end of the reaction when 0.75 moles of aluminum metal, (Al) and 0.50 moles of chlorine gas, (Cl ) 2re allowed to react as shown in the reaction below? a) 1.3 % b) 20 % c) 33 % d) 50 % e) 75 %
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